The Mole Concept
Christopher G. Hamaker, Illinois State University, Normal IL
© 2005, Prentice Hall
Avogadro’s Number
• Avogadro’s Number (symbol N) is the number of
atoms in 12.01 grams of carbon.
• Its numerical value is 6.02 × 1023.
• Therefore, a 12.01 g sample of carbon contains
6.02 × 1023 carbon atoms.
The Mole
• The mole (mol) is a unit of measure for an amount
of a chemical substance.
• A mole is Avogadro’s number of particles, that is
6.02 × 1023 particles.
1 mol = Avogadro’s Number = 6.02 × 1023 units
• We can use the mole relationship to convert
between the number of particles and the mass of a
substance.
How Big Is a Mole?
• The volume occupied by one mole of softballs
would be about the size of the Earth.
• One mole of Olympic shot put balls has about the
same mass as the Earth.
Mole Calculations
• We will be using the Unit Analysis Method again.
• Recall:
– First we write down the unit asked for
– Second we write down the given value
– Third we apply unit factor(s) to convert the given units
to the desired units
Mole Calculations I
• How many sodium atoms are in 0.120 mol Na?
– Step 1: we want atoms of Na
– Step 2: we have 0.120 mol Na
– Step 3: 1 mole Na = 6.02 × 1023 atoms Na
0.120 mol Na ×
6.02 × 1023 atoms Na
1 mol Na
= 7.22 × 1022 atoms Na
Mole Calculations I
• How many moles of potassium are in 1.25 × 1021
atoms K?
– Step 1: we want moles K
– Step 2: we have 1.25 × 1021 atoms K
– Step 3: 1 mole K = 6.02 × 1023 atoms K
1.25 ×
1021
atoms K ×
1 mol K
6.02 × 1023 atoms K
= 2.08 × 10-3 mol K
Molar Mass
• The atomic mass of any substance expressed in
grams is the molar mass (MM) of that substance.
• The atomic mass of iron is 55.85 amu.
• Therefore, the molar mass of iron is 55.85 g/mol.
• Since oxygen occurs naturally as a diatomic, O2,
the molar mass of oxygen gas is 2 times 16.00 g
or 32.00 g/mol.
Calculating Molar Mass
• The molar mass of a substance is the sum of the
molar masses of each element.
• What is the molar mass of magnesium nitrate,
Mg(NO3)2?
• The sum of the atomic masses is:
24.31 + 2(14.01 + 16.00 + 16.00 + 16.00) =
24.31 + 2(62.01) = 148.33 amu
• The molar mass for Mg(NO3)2 is 148.33 g/mol.
Mole Calculations II
• Now we will use the molar mass of a compound
to convert between grams of a substance and
moles or particles of a substance.
6.02 × 1023 particles = 1 mol = molar mass
• If we want to convert particles to mass, we must
first convert particles to moles and than we can
convert moles to mass.
Mass-Mole Calculations
• What is the mass of 1.33 moles of titanium, Ti?
• We want grams, we have 1.33 moles of titanium.
• Use the molar mass of Ti: 1 mol Ti = 47.88 g Ti
47.88 g Ti
1.33 mole Ti ×
= 63.7 g Ti
1 mole Ti
Mole Calculations II
• What is the mass of 2.55 × 1023 atoms of lead?
• We want grams, we have atoms of lead.
• Use Avogadro’s number and the molar mass of Pb
2.55 ×
1023
1 mol Pb
207.2 g Pb
atoms Pb ×
×
23
1 mole Pb
6.02×10 atoms Pb
= 87.8 g Pb
Mole Calculations II
• How many O2 molecules are present in 0.470 g of
oxygen gas?
• We want molecules O2, we have grams O2.
• Use Avogadro’s number and the molar mass of O2
1 mol O2
6.02×1023 molecules O2
0.470 g O2 ×
×
1 mole O2
32.00 g O2
8.84 × 1021 molecules O2
Gas Density
• The density of gases is much less than that of
liquids.
• We can calculate the density of any gas at STP
easily.
• The formula for gas density at STP is:
molar mass in grams
molar volume in liters
= density, g/L
Calculating Gas Density
• What is the density of ammonia gas, NH3, at STP?
• First we need the molar mass for ammonia;
– 14.01 + 3(1.01) = 17.04 g/mol
• The molar volume NH3 at STP is 22.4 L/mol.
• Density is mass/volume:
17.04 g/mol
22.4 L/mol
= 0.761 g/L
Molar Mass of a Gas
• We can also use molar volume to calculate the
molar mass of an unknown gas.
• 1.96 g of an unknown gas occupies 1.00L at STP.
What is the molar mass?
• We want g/mol, we have g/L.
1.96 g 22.4 L
×
= 43.9 g/mol
1.00 L 1 mole
Mole Unit Factors
• We now have three interpretations for the mole:
– 1 mol = 6.02 × 1023 particles
– 1 mol = molar mass
– 1 mol = 22.4 L at STP for a gas
• This gives us 3 unit factors to use to convert
between moles, particles, mass, and volume.
Mole-Volume Calculation
• A sample of methane, CH4, occupies 4.50 L at
STP. How many moles of methane are present?
• We want moles, we have volume.
• Use molar volume of a gas: 1 mol = 22.4 L
1 mol CH4
4.50 L CH4 ×
= 0.201 mol CH4
22.4 L CH4
Mass-Volume Calculation
• What is the mass of 3.36 L of ozone gas, O3, at
STP?
• We want mass O3, we have 3.36 L O3.
• Convert volume to moles then moles to mass:
1 mol O3
48.00 g O3
3.36 L O3 ×
×
22.4 L O3
1 mol O3
= 7.20 g O3
Molecule-Volume Calculation
• How many molecules of hydrogen gas, H2,
occupy 0.500 L at STP?
• We want molecules H2, we have 0.500 L H2.
• Convert volume to moles and then moles to
molecules:
1 mol H2
6.02×1023 molecules H2
×
0.500 L H2 ×
22.4 L H2
1 mole H2
= 1.34 × 1022 molecules H2
Law of Definite Composition
• The law of definite composition states that
“Compounds always contain the same elements in
a constant proportion by mass”.
• Sodium chloride is always 39.3% sodium and
60.7% chlorine by mass, no matter what its
source.
• Water is always 11.2% hydrogen and 88.8%
oxygen by mass.
Law of Definite Composition
A drop of water, a glass of water, and a lake of water all contain
hydrogen and oxygen in the same percent by mass.
Chemical Formulas
• A particle composed of two or more nonmetal
atoms is a molecule.
• A chemical formula expresses
the number and types of atoms
in a molecule.
• The chemical formula of
sulfuric acid is H2SO4.
Writing Chemical Formulas
• The number of each type of atom in a molecule is
indicated with a subscript in a chemical formula.
• If there is only one atom of a certain type, no ‘1’
us used.
• A molecule of the vitamin niacin has 6 carbon
atoms, 6 hydrogen atoms, 2 nitrogen atoms, and
1 oxygen atom. What is the chemical formula?
C6H6N2O
Interpreting Chemical Formulas
• Some chemical formulas use parenthesis to clarify
atomic composition.
• Antifreeze has chemical formula C2H4(OH)2.
There are 2 carbon atoms, 4 hydrogen atoms, and
2 OH units, giving a total of 6 hydrogen atoms
and 2 oxygen atoms.
• Antifreeze has a total of 10 atoms.
Percent Composition
• The percent composition of a compound lists the
mass percent of each element.
• For example, the percent composition of water,
H2O is:
– 11% hydrogen and 89% oxygen
• All water contains 11% hydrogen and 89%
oxygen by mass.
Calculating Percent Composition
• There are a few steps to calculating the percent
composition of a compound. Lets practice using
H2O.
– Assume you have 1 mole of the compound.
– One mole of H2O contains 2 mol of hydrogen
and 1 mol of oxygen.
– 2(1.01 g H) + 1(16.00 g O) = molar mass H2O
– 2.02 g H + 16.00 g O = 18.02 g H2O
Calculating Percent Composition
• Next, find the percent composition of water by
comparing the masses of hydrogen and oxygen in
water to the molar mass of water:
2.02 g H
× 100% = 11.2% H
18.02 g H2O
16.00 g O
× 100% = 88.79% O
18.02 g H2O
Percent Composition Problem
• TNT (trinitrotoluene) is a white crystalline
substance that explodes at 240°C. Calculate the
percent composition of TNT, C7H5(NO2)3.
• 7(12.01 g C) + 5(1.01 g H) + 3 (14.01 g N + 32.00 g O)
= g C7H5(NO2)3
• 84.07 g C + 5.05 g H + 42.03 g N + 96.00 g O
= 227.15 g C7H5(NO2)3.
Percent Composition of TNT
84.07 g C
× 100% = 37.01% C
227.15 g TNT
1.01 g H
× 100% = 2.22% H
227.15 g TNT
42.03 g N
× 100% = 18.50% N
227.15 g TNT
96.00 g O
× 100% = 42.26% O
227.15 g TNT
Empirical Formulas
• The empirical formula of a compound is the
simplest whole number ratio of ions in a formula
unit or atoms of each element in a molecule.
• The molecular formula of benzene is C6H6
– The empirical formula of benzene is CH.
• The molecular formula of octane is C8H18
– The empirical formula of octane is C4H9.
Calculating Empirical Formulas
• We can calculate the empirical formula of a
compound from its composition data.
• We can determine the mole ratio of each element
from the mass to determine the formula of radium
oxide, Ra?O?.
• A 1.640 g sample of radium metal was heated to
produce 1.755 g of radium oxide. What is the
empirical formula?
• We have 1.640 g Ra and 1.755-1.640 = 0.115 g O.
Calculating Empirical Formulas
• The molar mass of radium is 226.03 g/mol and the
molar mass of oxygen is 16.00 g/mol.
1 mol Ra
= 0.00726 mol Ra
1.640 g Ra ×
226.03 g Ra
1 mol O
= 0.00719 mol O
0.115 g O ×
16.00 g O
• We get Ra0.00726O0.00719. Simplify the mole ratio
by dividing by the smallest number.
• We get Ra1.01O1.00 = RaO is the empirical formula.
Empirical Formulas from
Percent Composition
• We can also use percent composition data to
calculate empirical formulas.
• Assume that you have 100 grams of sample.
• Benzene is 92.2% carbon and 7.83% hydrogen,
what is the empirical formula.
• If we assume 100 grams of sample, we have
92.2 g carbon and 7.83 g hydrogen.
Empirical Formulas from
Percent Composition
• Calculate the moles of each element:
1 mol C
= 7.68 mol C
92.2 g C ×
12.01 g C
7.83 g H ×
1 mol H
= 7.75 mol H
1.01 g H
• The ratio of elements in benzene is C7.68H7.75.
Divide by the smallest number to get the formula.
C
7.68
7.68
H
7.75
7.68
= C1.00H1.01 = CH
Molecular Formulas
• The empirical formula for benzene is CH. This
represents the ratio of C to H atoms of benzene.
• The actual molecular formula is some multiple of
the empirical formula, (CH)n.
• Benzene has a molar mass of 78 g/mol. Find n to
find the molecular formula.
(CH)n
78 g/mol
=
CH
13 g/mol
n = 6 and the molecular
formula is C6H6.
Conclusions
• Avogadro’s number is 6.02 × 1023 and is one mole
of any substance.
• The molar mass of a substance is the sum of the
atomic masses of each element in the formula.
• At STP, 1 mole of any gas occupies 22.4 L.
Conclusions Continued
• We can use the following flow chart for mole
calculations:
Conclusions Continued
• The percent composition of a substance is the
mass percent of each element in that substance.
• The empirical formula of a substance is the
simplest whole number ratio of the elements in the
formula.
• The molecular formula is a multiple of the
empirical formula.